A solution containing a mixture of metal cations was treated as follows. 1. Dilute HCl was added and a precipitate formed. The precipitate was filtered off. 2. H2S was bubbled through the acidic solution. Again, a precipitate formed and was filtered off. 3. The pH was raised to about 9 and H2S was again bubbled through the solution. No precipitate formed. 4. Finally, sodium carbonate was added and no precipitate formed. What can be said about the presence of each of these groups of cations in the original solution?

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Essence Fritz

Chemistry

6 October, 06:45

A solution containing a mixture of metal cations was treated as follows. 1. Dilute HCl was added and a precipitate formed. The precipitate was filtered off. 2. H2S was bubbled through the acidic solution. Again, a precipitate formed and was filtered off. 3. The pH was raised to about 9 and H2S was again bubbled through the solution. No precipitate formed. 4. Finally, sodium carbonate was added and no precipitate formed. What can be said about the presence of each of these groups of cations in the original solution?

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Johan Acevedo · Answer 1

None of the listed atoms are definitely present, as there is no way to tell from the limited information. Likewise, we know from the chart of the seperation of cations that Ba2 + and Ca2 + have no chance of being there, since they form precipitates when carbonate is added. Ag+, Pb2+, and Hg2^2 + have no chance of being there either, since they form precipitates when dilute HCl is first added. The rest on the list are all possibly